0.1 m solutions of sodium sulphate,urea,and | vedclass

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(B) The elevation in boiling point $(\Delta T_b)$ is given by the formula: $\Delta T_b = i 	imes K_b 	imes m$.Since the molality $(m)$ and the ebull

Vedclass · Accepted Answer

$3 : 1 : 2$

Vedclass · Answer

(B) The elevation in boiling point $(\Delta T_b)$ is given by the formula: $\Delta T_b = i 	imes K_b 	imes m$.Since the molality $(m)$ and the ebullioscopic constant $(K_b)$ are the same for all solutions,$\Delta T_b$ is directly proportional to the van't Hoff factor $(i)$.For $Na_2SO_4$ (sodium sulphate),$i = 3$ (as it dissociates into $2Na^+ + SO_4^{2-}$).For urea (a non-electrolyte),$i = 1$.For $NaCl$ (sodium chloride),$i = 2$ (as it dissociates into $Na^+ + Cl^-$).Therefore,the ratio of the elevation in boiling point is $3 : 1 : 2$.

$0.1 \ m$ solutions of sodium sulphate,urea,and sodium chloride are taken. The correct ratio of the elevation of boiling point of these solutions is

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